Answer
$0.30\,kJ/mol$
Work Step by Step
We obtain the required reaction by reversing the second reaction and then adding the first reaction with it.
Therefore, $\Delta H^{\circ}_{rxn}=-[\Delta H^{\circ}(\text{second reaction)}]+[\Delta H^{\circ}(\text{first reaction})]$
$=-(-296.36\,kJ/mol)+(-296.06\,kJ/mol)=0.30\,kJ/mol$
